Calculate the [H*] in a solution that has a pH of 9.16.

Q: Calculate the pH of a 0.100 M KCN solution.

A: Anionic part of the salt will be hydrolysed and cationic part of the salt will not be hydrolysed.

Q: What is the pH of a solution that has [H3O*]= 4.5x10-³ M?

A:

Q: Calculate the [H+] or [H3O+] in a solution that has a pH of 8.75.

A: Given: pH = 8.75.

Q: [H;O'] [OH'] pH pOH acidic or basic ? 1.7 X 10:1ºM 8.79

A: pH = -log[H+] pOH = -log[OH-] pH+pOH = 14 If pH>7, basic If pH<7, acidic

Q: 12) The pH of a solution is measured to be 10.40. What are the values of [H3O+] and [OH-] for this…

A: The pH of the solution = 10.40 H3O+=?OH-=?

Q: Solution A has a pH of 5.6. Solution B has a pH of 2.8. Which has a higher (H*] concentration? O…

A:

Q: Which of the following can be classified as a Lewis base? BH3 O I only II, III, and IV O I and II O…

A: Lewis bases are those compounds which has lone pair of electrons to donate.  Lewis acids are those…

Q: A certain weak base has a ?bKb of 8.80×10−7.8.80×10−7. What concentration of this base will produce…

A: 0.057 M

Q: concentration

A: [H+] = 10^-pH  [H+] = 10^-1.80  [H+] = 0.0158 M

Q: Type your answers in all of the blanks and submit Answer the following questions to review the…

A: In a neutral water the concentration of hydrogen ion and hydroxide ion are equal and the…

Q: Find the pH of a solution with a hydroxide ion concentration of 0.025M.

A: hydroxide ion concentration (OH-) = 0.025M.

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0104 M solution. The pH of the…

A: Given, pH of the solution is 2.63 and the concentration is 0.0104M We can determine the Ka using the…

Q: Calculate the [H+] in a solution that has a pH of 3.19

A: In this question, we will calculate the [H+] Concentration from the given pH of the Solution. How we…

Q: Question 3 A student is given a concentrated solution that is supposed to contain vinegar, a weak…

A: A weak acid will not be completely dissociated in a solution. However, a strong acid will be…

Q: The pH of an acidic solution is 2.11. What is [H*]?

A:

Q: What are [H*], [OH-] and pH in a solution with a pOH of 12.11 15.

A:

Q: The pOH of an aqueous solution at 25°C was found to be 4.90. The pH of this solution is . The…

A: Note : Since you have posted multiple questions , as per guidelines we can solve only 1 . To get the…

Q: Calculate the [H+] in a solution that has a pH of 9.88.

A: pH of any solution is the potential of hydrogen ions . It is given by :pH = -log[H+ ] where [H+ ] =…

Q: nough of a monoprotic acid is dissolved in water to produce a 1.60 M solution. The pH of the…

A:

Q: Aspirin, which is acetylsalicylic acid, was the first NSAID used to alleviate pain and fever. If a…

A: Introduction If the value of hydronium ion of any particular solution is known then one can easily…

Q: What is the pH of a solution in which 15 mL of 0.38 M NaOH is added to 25 mL of 0.38 M HCl? pH =

A: Given -> Molarity of NaOH= M1 = 0.38 M  Volume of NaOH= V1 = 15 ml  Molarity of HCl = M2 = 0.38 M…

Q: An unknown weak acid with a concentration of 0.088 M has a pH of 1.80. What is the Ka of the weak…

A: Since it is not given whether the weak acid is monoprotic or polyprotic. Hence I'm assuming the acid…

Q: Enough of a monoprotic acid is dissolved in water to produce a 0.0162 M solution. The pH of the…

A: Given,  The concentration of monoprotic acid = 0.0162 M.  The pH of the solution = 2.57. The Ka of…

Q: Calculate the hydroxide ion concentration of a solution with pH = 6,4.

A: pH of solution is 6.4 We need to determine [OH-]

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0114 M solution. The pH of the…

A: Answer:Ostwald's dilution law is applicable for weak acids and its gives as a relation between…

Q: What is the pH of a bleach solution that has a [OH-| = 2.4 x 10-5 M? pH = Is bleach acidic, basic,…

A:

Q: pH is a logarithmic scale used to indicate the hydrogen lon concentration, [H], of a solution: pH =…

A: Given :  For part A :  Mass of HCl = 0.55 g  Volume of solution = 5.5 L   For part B :  Mass of NaOH…

Q: what is the pH of the solution if 16.0 mL of 0.100 M NaOH is added to 20.0 mL of 0.150 M HCl? Is the…

A:

Q: 2. An aqueous solution has a pH of 3.75. What is the hydronium ion concentration of the solution? Is…

A: We have to predict the hydronium ion concentration and nature of solution .

Q: The pH of normal rain water is 5.80. What will be the pH of rainwater that falls near a coal-burning…

A: pH  is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions  are…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.